calculate the pH of a 1.25 x 10^-3 M HNO3 solution
This is hardly organic chemistry.
(HNO3) = 1.25E-3M.
Since HNO3 is a strong acid (100% ionized), that means (HNO3) = (H^+); therefore, (H^+) = 1.25E-3 and
pH = -log(H^+) = -log(1.25E-3) = ?? The answer is approximately 3
To calculate the pH of a solution, you need to know the concentration of hydrogen ions (H+). In this case, we have a 1.25 x 10^-3 M HNO3 solution. Since HNO3 is a strong acid, it completely ionizes in water to form H+ ions.
The concentration of H+ ions in the HNO3 solution is equal to the concentration of the acid itself because it completely dissociates. Therefore, we can say that the concentration of H+ ions is 1.25 x 10^-3 M.
The pH of a solution is defined as the negative logarithm (base 10) of the hydrogen ion concentration. Mathematically, it is expressed as pH = -log[H+].
Let's plug in the value of the H+ concentration into the equation:
pH = -log(1.25 x 10^-3)
Now, using a scientific calculator or an online calculator, we can calculate the pH:
pH ≈ -(-2.903)
pH ≈ 2.903
Therefore, the pH of a 1.25 x 10^-3 M HNO3 solution is approximately 2.903.